Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial mass of key (g) 8.464g Final mass of key (g) 8.525g Average current (A) 0.015 A Time of current application (s) 30 min   Use your data from measuring the mass of the electrode and the key to calculate the actual number of moles of copper that plated out.

Q: Silver is deposited on a metallic vessel of surface area 800 cm2 by passing current of 0.2 ampere,…

A: By Faraday's law: Mass of silver deposited (w): w = E×I×t96500 =108×0.2×3×360096500=2.42 g  Mass of…

Q: Part A. How many seconds are required to deposit 0.123 grams of tin metal from a solution that…

A: Faraday's law in electrolysis:

Q: PART A. Cell Potentials Negative Electrode Electrode E° cell Anode E° anode Cathode E° cathode…

A: The main equation to solve this question is: E0cell=E0reduction-E0oxidation Now, At cathode:…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current of 1.24 A to plate…

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Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A:

Q: A “dead” 12-Volt lead/acid storage battery has 12.80 g of PbSO4 (molar mass = 303.3 g), deposited on…

A: According to Faraday's first of electrolysis, the amount of substance liberated at a particular…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate…

A:

Q: A potential of - 0.788 V is applied to a cell with Nernst Potential of -0.734 V. The internal…

A: We need to find the overpotential.

Q: The formation of green patina (copper carbonate) on a copper roof protecting the underlying copper…

A: B) Cathodic protection : It is a process by which the corrosion of a metal surface is controlled by…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.55 minutes for a current…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.02 minutes for a current…

A:

Q: Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial…

A: Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial mass…

Q: Electrolytic Reduction of Cu2+ to Cu on the Surface of a Coin initial mass of coin: 5.6917 g…

A: Given: The initial mass of coin=5.6917 g The final mass of coin=5.7553 g    Coulombs…

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.57 minutes for a current…

A: A numerical problem based on electrolysis that is to be accomplished.

Q: ELECTROCHEMISTRY: Copper was electroplated from a Cu2SO4 solution onto an electrode with an active…

A: Cu2SO4 is used for electroplating 7.73cm2 area using current of 4.54A for 0.6978 hours.

Q: A “dead” 12-Volt lead/acid storage battery has 4.30 g of PbSO4 (molar mass = 303.3 g), deposited on…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.52 minutes for a current…

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Q: Determine the mass of Sodium (Na) produced when a 295 amp current flows for 8 hr through a cell…

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Q: What is the initial cell potential? Express your answer using two decimal places. HA ? Ecell =…

A: We have to find the E cell of given reaction

Q: Galvanized nails are iron nails that have been plated with zinc to prevent rusting. The relevant…

A:

Q: The gold plating of a ceramic figurine requires a total of 4.96 g of solid gold. If the current…

A: Given,  Mass of gold required, w = 4.96 g  Current passed, I = 11.8 A  Molar mass of gold = 197…

Q: A baby's spoon with an area of 6.25 square centimeter is plated with silver from silver nitrate…

A: Faraday's Laws of electrolysis establishes the relationship between mass of the substance…

Q: Initial mass of copper electrode (g) 1.201g Final mass of copper electrode (g) 1.163g Initial…

A: Given information: Initial mass of copper electrode (g) = 1.201g Final mass of copper electrode (g)…

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.66 minutes for a current…

A:

Q: An object with a surface area of 85.5 cm? is to be plated with nickel. A current of 7.95 A is…

A: This question is based on the Faradays second law of electricity. It states that the number of…

Q: A spoon is to be electroplated with Ag(s) using a solution containing Ag+ ions. If 32.4 grams of…

A: The amount of substance deposited on the electrode on passing electric current is given by the…

Q: Use the standard potential data available in the literature and design a cell with a theoretical…

A: Electrochemical cell is the device which is used to convert electrical energy into chemical energy…

Q: A baby’s spoon with an area of 6.25 square centimeter is plated with silver from silver  nitrate…

A: Since you have asked multiple questions questions, we will solve the first question for you. If you…

Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…

A:

Q: Initial mass of copper (g) 5.720 Average current (A) 0.386A Final mass of copper (g)…

A: 1. Formula for total charge passed through an electrolytic cell = current × time = 0.386 A × 30.0×60…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.12 minutes for a current…

A: Given: Time = 1.12 minutes = 1.12×60 sec Correct = 1.22 A Mass of the metal M = 0.0896 g

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Answer  = 3.50 grams

Q: 18 « < 4 o Object Object AGNO3(aq) Zn(NO3)2(aq) Diagram 1 Diagram 2 Object Metal Used Amount of…

A: Explanation to the correct option is given below.

Q: A student deposited 2.50 g of zinc (65.39 g/mol) onto a sculpture from a ZnSO4 solution. The…

A: Given that : The mass of zinc deposited = 2.50 g Molar mass of Zn = 65.39 g/mol Current supplied =…

Q: The partial pressure in atm required for half-cells that generate or consume gas for its standard…

A: The standard state of half cell:  The standard state of half cell is when the partial pressure of a…

Q: The gold plating of a ceramic figurine requires a total of 4.19 g of solid gold.  If the current…

A: Given  Mass of solid gold required = w = 4.19 g Current being used is = I = 11.0 amperes how many…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.57 minutes for a current…

A: Using the formula for mass deposition to solve this.

Q: One type of iron nail is coated with another metal in order to reduce corrosion. A solution of the…

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Q: Determine the mass of Sodium( Na) produced when a 10 amp current flows for 4 hr through a cell…

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Q: What happens during the discharge of a lead-acid battery? A. The negative plate forms lead sponge.…

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Q: Magnesium metal is to be produced from the electrolysis of molten magnesium bromide. MgBr½(1) →…

A: Electrolysis of MgBr2 whose amount of Mg produced is to be determined.

Q: Example 8. A 100 watt, 110 volt incandescent lamp is con- nected in series with an electrolytic cell…

A: Given: power=100 wattvoltage=110 volttime=10 hours To find: Mass of cadmium

Q: A voltaic cell is constructed with two Zn2+-Zn electrodes. The two cell compartments have [Zn2+]…

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Q: object with a surface area of 24.1 cm224.1 cm2 is to be plated with nickel. A current of 7.93 A7.93…

A: The total volume covered by Nickel=surface area×thickness of Nickel layer=24.1 cm2×9.71×10-3cm0.234…

Q: A baby'sspoon with an area of 6.25 cm2 is plated with silver from AgN03 using a current of 2.00 A…

A: (a),

Q: Calculate the time required for a constant current of 0.951 A to deposit 0.205 g of Co(II) in the…

A: (a) . Suppose a half cell reaction is : Co2+ + 2 e-  ↔ Cos To calculate the time required for a…

Q: A “dead” 12-Volt lead/acid storage battery has 13.00 g of PbSO4 (molar mass = 303.3 g), deposited on…

A: According to Faraday’s first law of electrolysis,

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.